91Ó°ÊÓ

Which of the following statements is/are true regarding a \(1.0 M\) solution of a strong acid HA? (a) \(\left[\mathrm{A}^{-}\right]>\left[\mathrm{H}^{+}\right]\) (b) The pH is 0.00 . (c) \(\left[\mathrm{H}^{+}\right]=1.0 M\) (d) \([\mathrm{HA}]=1.0 \mathrm{M}\)

What does the ionization constant tell us about the strength of an acid?

List the factors on which the \(K_{\mathrm{a}}\) of a weak acid depends.

Why do we normally not quote \(K_{\mathrm{a}}\) values for strong acids such as \(\mathrm{HCl}\) and \(\mathrm{HNO}_{3}\) ? Why is it necessary to specify temperature when giving \(K_{\mathrm{a}}\) values?

Which of the following solutions has the highest pH: (a) 0.40 M HCOOH, (b) \(0.40 M \mathrm{HClO}_{4}\), (c) \(0.40 \mathrm{M} \mathrm{CH}_{3} \mathrm{COOH} ?\)

The \(K_{\mathrm{a}}\) for benzoic acid is \(6.5 \times 10^{-5} .\) Calculate the \(\mathrm{pH}\) of a \(0.10 \mathrm{M}\) benzoic acid solution.

A 0.0560-g quantity of acetic acid is dissolved in enough water to make \(50.0 \mathrm{~mL}\) of solution. Calculate the concentrations of \(\mathrm{H}^{+}, \mathrm{CH}_{3} \mathrm{COO}^{-},\) and \(\mathrm{CH}_{3} \mathrm{COOH}\) at equilibrium. \(\left(K_{\mathrm{a}}\right.\) for acetic acid \(\left.=1.8 \times 10^{-5} .\right)\)

A \(0.040 M\) solution of a monoprotic acid is 14 percent ionized. Calculate the ionization constant of the acid.

Which of the following has a higher pH: (a) \(0.20 \mathrm{M}\) \(\mathrm{NH}_{3},\) (b) \(0.20 \mathrm{M} \mathrm{NaOH} ?\)

Calculate the \(\mathrm{pH}\) of a \(0.24 \mathrm{M}\) solution of a weak base with a \(K_{b}\) of \(3.5 \times 10^{-6}\) .